ICSE Class 10 Chemistry Syllabus 2026-27 — Complete Guide with Marks Distribution & Tips

What's New in 2026-27?

The ICSE Class 10 Chemistry syllabus for 2026-27 continues to emphasise both theoretical concepts and practical applications. CISCE has maintained the focus on analytical chemistry (laboratory tests for gases and acids), stoichiometry, and organic chemistry fundamentals. The competency-based assessment approach means students should expect questions that test application of concepts to real-world scenarios, particularly in the Study of Compounds and Organic Chemistry units.

Chemistry (Science Paper 2) carries 80 marks for the theory examination and 20 marks for Internal Assessment (practical work). Duration: 2 hours.

Syllabus Overview

Unit	Topics	Approximate Marks
Periodic Table	Modern periodic table, periodicity of properties, groups and periods	~6 marks
Chemical Bonding	Electrovalent and covalent bonding, properties of compounds	~6 marks
Acids, Bases and Salts	Definitions, pH scale, indicators, preparation of salts	~8 marks
Analytical Chemistry	Identification of gases, action of acids on salts	~4 marks
Mole Concept & Stoichiometry	Mole, Avogadro's number, balancing equations, calculations	~8 marks
Electrolysis	Electrolytes, electrodes, electrolysis of solutions, electroplating	~8 marks
Metallurgy	Extraction of aluminium and iron, alloys	~6 marks
Study of Compounds	HCl, NH₃, HNO₃, H₂SO₄ — preparation, properties, uses	~20 marks
Organic Chemistry	Hydrocarbons, alcohols, carboxylic acids, homologous series	~10 marks

Chapter-wise Detailed Syllabus

1. Periodic Table (~6 marks)

Modern periodic table — periods and groups, atomic number as basis of classification. Periodicity of properties: atomic size, metallic character, non-metallic character, ionisation potential, electron affinity, electronegativity. Trends across periods and down groups. Students should be able to predict properties of elements based on their position.

2. Chemical Bonding (~6 marks)

Electrovalent (Ionic) Bonding: Transfer of electrons, formation of ions, conditions for ionic bond formation, properties of ionic compounds (high MP, conduct electricity in molten/solution state).

Covalent Bonding: Sharing of electrons, single, double, triple bonds. Electron dot structures. Properties of covalent compounds (low MP, poor conductors). Polar and non-polar covalent bonds.

3. Acids, Bases and Salts (~8 marks)

Definitions (Arrhenius, Bronsted-Lowry), strong and weak acids/bases, pH scale and indicators (litmus, phenolphthalein, methyl orange, universal indicator). Preparation of normal salts, acid salts, and basic salts. Action of dilute acids on metals, carbonates, and bases.

4. Analytical Chemistry (~4 marks)

Identification of gases — hydrogen, oxygen, carbon dioxide, chlorine, hydrogen chloride, sulphur dioxide, hydrogen sulphide, ammonia, water vapour, nitrogen dioxide. Tests include colour, odour, effect on indicators, and specific chemical tests. This is a highly practical and scoring section.

5. Mole Concept and Stoichiometry (~8 marks)

Mole concept — Avogadro's number (6.022 × 10²³), molar mass, molar volume at STP (22.4 L). Balancing chemical equations. Stoichiometric calculations — relating moles, mass, and volume. Percentage composition, empirical and molecular formulae. Gay-Lussac's law of combining volumes.

6. Electrolysis (~8 marks)

Electrolytes (strong and weak), non-electrolytes. Electrolysis of acidulated water, copper sulphate solution (with copper and platinum electrodes), molten lead bromide. Selective discharge of ions. Electroplating — process and applications. Electrode reactions (oxidation at anode, reduction at cathode).

7. Metallurgy (~6 marks)

Extraction of Aluminium: Purification of bauxite (Bayer's process), electrolytic reduction (Hall-Heroult process), role of cryolite and fluorspar.

Extraction of Iron: Blast furnace — charge, zones (combustion, reduction, slag formation), reactions at each zone. Alloys — composition and uses of steel, brass, bronze, duralumin.

8. Study of Compounds (~20 marks — Highest Weightage)

This is the most important unit in ICSE Chemistry, carrying the highest marks. Students must thoroughly study:

• Hydrogen Chloride (HCl): Laboratory preparation from NaCl and H₂SO₄, drying, collection (upward displacement). Properties — dense, fuming, acidic. Fountain experiment. Aqueous solution properties.
• Ammonia (NH₃): Laboratory preparation from NH₄Cl and Ca(OH)₂. Properties — alkaline, lighter than air. Haber's process for industrial manufacture. Ammonium salts.
• Nitric Acid (HNO₃): Laboratory preparation, Ostwald's process for industrial manufacture. Properties — oxidising agent, action on metals (Cu, Fe) and non-metals (C, S). Aqua regia.
• Sulphuric Acid (H₂SO₄): Contact process for manufacture. Properties — dehydrating agent, oxidising agent, sulphonating agent. Dilute vs. concentrated behaviour. Action on metals.

9. Organic Chemistry (~10 marks)

Introduction: Unique properties of carbon (tetravalency, catenation), homologous series — definition, characteristics, general formula.

Hydrocarbons: Alkanes (CₙH₂ₙ₊₂), alkenes (CₙH₂ₙ), alkynes (CₙH₂ₙ₋₂). IUPAC nomenclature, structural formulae. Methane — preparation and properties. Ethylene — preparation and properties (addition reactions).

Alcohols: Methanol and ethanol — preparation, properties, uses. Denatured spirit.

Carboxylic Acids: Acetic acid — preparation, properties (esterification, reaction with bases). Vinegar.

Exam Pattern 2026-27

Component	Details	Marks
Section I	Compulsory short-answer questions from all units	40 marks
Section II	Answer 4 out of 6 structured/long-answer questions	40 marks
Internal Assessment	Practical work, project, periodic tests	20 marks
Total		100 marks

Prescribed Textbooks

• Concise Chemistry Class 10 — Selina Publishers
• Dalal ICSE Chemistry Class 10 — Allied Publishers
• Viraf Dalal Simplified ICSE Chemistry — commonly used reference
• CISCE specimen papers and previous years' board papers

Preparation Tips

1. Master Study of Compounds first — With ~20 marks, this is the highest-weightage unit. Learn the preparation, properties, and uses of HCl, NH₃, HNO₃, and H₂SO₄ thoroughly. Write chemical equations from memory.
2. Practise balancing equations daily — Stoichiometry requires balanced equations as the foundation. Practise balancing 5 equations daily until it becomes automatic.
3. Create gas identification charts — Make a table of all gases with their colour, odour, test, and result. This is the easiest scoring section if you memorise the tests.
4. Draw electron dot structures — For Chemical Bonding, practise drawing electron dot structures for NaCl, MgCl₂, CaCl₂, H₂O, CO₂, NH₃, CH₄, and C₂H₄.
5. Learn organic chemistry naming — IUPAC nomenclature is systematic. Learn the rules and practise naming 20+ compounds. This saves time in the exam.
6. Solve mole concept numericals — Mole concept problems follow a pattern. Practise converting between moles, mass, volume, and number of particles until it's second nature.
7. Revise metallurgy diagrams — Draw and label the blast furnace and Hall-Heroult cell diagrams. These are frequently asked for 3-4 marks.